Multiple Choice
A mixture of CaCO₃ and CaO has a mass of 2.5000 g. After heating, the mass of the sample is reduced to 2.016 g due to the decomposition of CaCO₃ into CaO and CO₂. What is the mass percent of CaCO₃ in the original mixture?
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3. Chemical Reactions
Stoichiometry
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According to the balanced equation 3 NO2(g) + H2O(l) ⟶ 2 HNO3(aq) + NO(g), how many moles of NO are formed from 8.44 moles of NO2 if there is plenty of water present?
A
4.22 moles
B
2.81 moles
C
5.63 moles
D
8.44 moles
Verified step by step guidance1
Identify the balanced chemical equation: 3 NO2(g) + H2O(l) ⟶ 2 HNO3(aq) + NO(g).
Determine the mole ratio between NO2 and NO from the balanced equation. The coefficients indicate that 3 moles of NO2 produce 1 mole of NO.
Set up a proportion using the mole ratio to find the moles of NO produced from 8.44 moles of NO2. Use the equation: (3 moles NO2 / 1 mole NO) = (8.44 moles NO2 / x moles NO).
Solve the proportion for x, which represents the moles of NO produced.
Verify the calculation by checking that the units cancel appropriately and the result makes sense in the context of the problem.
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